* Solid State: In their solid state, ionic compounds form a rigid lattice structure. The ions are held tightly in place by strong electrostatic forces. This fixed arrangement prevents the free movement of ions, which is necessary for electrical conductivity.
* Aqueous Solution: When an ionic compound dissolves in water, the water molecules surround the ions and pull them apart, breaking the lattice structure. These free ions are now able to move throughout the solution, carrying an electric current.
* Molten State: When an ionic compound is heated to its melting point, the strong electrostatic forces holding the ions together are weakened, allowing the ions to move freely. This free movement of ions enables the molten compound to conduct electricity.
In summary, ionic compounds only conduct electricity when their ions are free to move. This occurs in aqueous solutions and molten states.
